The correct answer is option 4, that is, an ionic compound.
The mentioned features belong to an ionic compound. The ionic compounds exhibit strong bonds in between their atoms, that is, an ionic bond is the strongest molecular bond, this confirms that ionic compounds exhibit a high melting point.
The ionic compounds do not transmit current, as they do not possess free electrons, like metals, thus, they are poor conductors as solid. The ionic compounds get dissolve in water and form ions that are the charges, which can move, making them good conductors as a liquid. The composition of the ionic compound is a set of crystals that makes them brittle and hard.
Answer:
Explanation:
All the colligatives properties are modified by the Van't Hoff factor. This is shown as i, in the formula of the colligative properties freezing point depression, boiling point elevation, and osmotic pressure.
The Van't Hoff factor shows the number of particles into which the solute dissociates. In organic compounds we use 1, in inorganic compounds we have to think the dissociation. For example in aquous solutions, inorganic salts as AgNO₃ and CaCl₂ dissociate like this:
AgNO₃ → Ag⁺ + NO₃⁻
CaCl₂ → Ca²⁺ + 2Cl⁻
AgNO₃ has 2 moles of ions and CaCl₂ has 3 moles.
In urea: i = 1
In silver nitrate: i = 2
In calcium chloride: i = 3
The i = 3 for calcium chloride, makes that this salt has the highest osmotic pressure, highest vapor pressure and highest boiling point.
Answer:
107.5 amu
Explanation:
isotopes: fractional Wt Avg
isotopes: isotopic mass %Abundance abundance (amu)
X110 110 60 0.60 66.0
X105 105 30 0.30 31.5
<u> X100 100 10 0.10 10.0</u>
∑ atm mass contributions = 107.5 amu*
*amu = atomic mass units
Answer:
The compound is ionic
The compound has a high melting point
The compound will conduct electricity in aqueous solution
The compound will be soluble in water
Explanation:
Now, let us consider the nature of the compound formed when a metal X looses two electrons and a non metal Y accepts one electron.
The compound formed must be ionic in nature with a formula XY2. Ionic compounds are formed by transfer of electrons from metals to nonmetals.
The ionic substance formed is always soluble in water with a high melting point. Usually, ionic solids do not conduct electricity in the solid state because the charge carriers (ions) are tightly bound in the crystal structure while in the solid state. In aqueous solution, the ions are relatively free hence ionic substances conduct electricity in aqueous solution.
